Acids and Bases key terms

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alkaline
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the solution formed when a base completley dissociates in water to yield aqueous OH- ions
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arrhenius acid
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a chemical compound that increases the concentration of hydrogen ions, H+, in aqueous solutions
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arrhenius base
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a substance that increases the concentration of hydroxide ions, OH-, in aqueous solutions
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binary acid
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an acid that contains only two different elements: hydrogen and one of the more electronegtive elements
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oxyacid
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an acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal
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strong acid
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one that ionizes completley in aqueous solutions
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weak acids
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acids that are weak electrolytes
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amphoteric
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any species that can react as either an acid or a base
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Bronsted-Lowry acid
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is a molecule or ion that is a proton donor
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Bronsted-Lowry Base
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is a molecule or ion that is a proton acceptor
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Bronsted-Lowry Acid-base reactions
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protons are transferred from one reactant (the acid) to another (the base)
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monoprotic acid
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an acid that can donate only one proton (hydrogen ion) per molecule
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polyprotic acid
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ana tom that can donate more than one proton per molecule
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diprotic acid
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can donate two protons per molecule
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triprotic acid
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an acid able to donate three protons per molecule
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Lewis acid
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an atom, ion, or molecule that accepts an electron pair to form a covalent bond
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Lewis base
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an atom, ion, or molecule that donates an electron pair to form a covalent bond
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Lewis acid-base reaction
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the formation of one or more covalent bonds between an electron-pair donor and electron pair acceptor
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conjugate base
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the species left after a Bronsted-Lowry acid has given up a proton
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Conjugate acid
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species left after a Bronsted-Lowry base gains a proton
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neutralization
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the reaction of hydronium ions and hyroxide ions to form water molecules
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salt
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ionic compound composed of a cation rom a base and an anion from an acid

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